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Science Clinic => Chemistry => Topic started by: Kikoku on Nov 18, 2019

Title: Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 ...
Post by: Kikoku on Nov 18, 2019

Question 1

According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g mol-1, H2O = 18.02 g mol-1.
Al2S3(s) + 6H2O(l) → 2Al(OH)3(s) + 3H2S(g)

◦ 14.00 g
◦ 28.33 g
◦ 17.22 g
◦ 19.78 g
◦ 8.33 g

Question 2

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2.

2C8H18 + 25O2 → 16CO2 + 18H2O

◦ 25.00%
◦ 50.00%
◦ 20.00%
◦ 12.50%

Title: Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 ...
Post by: jaaaaaaa on Nov 18, 2019

Answer 1

17.22 g

Answer 2

25.00%

Title: Re: Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8
Post by: clairethomsonn on Sep 22, 2021

thank you